Molar Mass
The molar mass is useful when converting between _______________ and ______________.
What is grams and moles?
This is the procedure for converting from grams to moles.
Divide by (put on bottom) the molar mass.
This is the definition of a limiting reagent.
(Something like . . .)
What is the chemical that gets used up first in a reaction. It is the chemical that limits how much product you can make.
This is the equation for calculating percent yield.
What is Percent yield = (actual yield / theoretical yield) x 100
Chemical equations must be balanced to obey this law
What is The Law of Conservation of Mass?
This is the molar mass of Na.
What is 22.99 g/mole?
This is the 'path' to convert from Grams Given to Grams Wanted
What is
Grams to Moles
Moles to Moles
Moles to Grams
If you're making ham sandwiches. Each sandwich needs 2 pieces of bread and one slice of ham. If you have 30 pieces of bread and 20 slices of ham, this is the limiting reagent.
What is the bread?
If you got 45 out of 50 possible questions right on a test, this was your % score.
What is 90 %
This side of the equation shows the reactants
What is the left side?
This is the molar mass of Li2S.
What is 46 g/mole?
Fe2O3 + CO2 --> 2Fe + 3CO2
This much Fe2O3 is needed to produce 92.8 g of Fe
What is 133 g Fe2O3
2Cu + S --> Cu2S
This is the limiting reactant when 80 g of Cu reacts with 25 g of S.
What is copper?
If you actually produced 12.8 grams of a substance, but theoretically expected 13.6 grams, this was your percent yield.
What is 94%.
This is calculated using actual and theoretical yields.
What is percent yield?
This is the molar mass of Na3PO4.
What is 164 g/mole?
2NaOH + CO2 --> Na2CO3 + H2O
This number of grams of CO2 are needed to react with 3.50 grams of NaOH.
What is 1.93 g CO2?
If you got 87% yield when you made 15.7 grams of a substance, what was your theoretical yield?
What is 18 g?
CaCO3 --> CaO + CO2
This is the theoretical yield of CaO if 24.8 g of CaCO3 is decomposed?
What is 13.9 g of CaO.
This is the amount of particles in 1 mole.
What is 6.02 x 1023 ?
In the equation:
2Fe2O3 + C --> Fe + 3CO2,
this is the molar mass of carbon dioxide.
What is 44 g/mole?
SiO2 + 3C --> SiC + 2CO
When 50 g of silicon dioxide is heated with an excess of carbon, it should produce this many grams of silicon carbide.
What is 33.38g SiC?
N2H4 + O2 --> N2 + 2 H2O
You have 1,000 g of N2H4 and 1,400 g of O2.
How many grams of the excess reagent will remain after the reaction?
What is 400 grams excess O2
1 - Determine the limiting reactant
2 - Use that limiting amount to determine how much of the excess is used.
3 - Subtract from the amount of excess reagent you began with.
4FeCO3 + O2 --> 2Fe2O3 +4CO2
In the lab, 75 g of FeCO3 is heated with an excess of oxygen and 45 g of Fe2O3 is produced.
This is the percent yield of the reaction
What is 87.06%
This causes the reaction to stop
What is the Limiting Reagent / Reactant?